ULTRASONIC STUDY OF INTERMOLECULAR ASSOCIATION THROUGH HYDROGEN BONDING IN TERNARY LIQUID MIXTURES

ULTRASONIC STUDY OF INTERMOLECULAR ASSOCIATION THROUGH HYDROGEN BONDING IN TERNARY LIQUID MIXTURES S. Thirumaran 1 and Deepesh George 1 Department of Physics (DDE), Annamalai University, Annamalainagar, India E-Mail: thiru_phymaran@yahoo.co.in ABSTRACT The ultrasonic velocity, density and viscosity have been measured for the liquid mixtures of cresols namely, m- cresols, o-cresols and p-cresols with N,N-Dimethyl formamide (DMF) in CCl 4 at 303, 308 and 313 K. The experimental data have been used to calculate the acoustical parameters such as adiabatic compressibility (β), free length (L f ), free volume (V f ), internal pressure (π i ), acoustic impedance (Z) and molar volume (V m ). The excess values of some of the above parameters have also been evaluated and fitted to Redlich-Kister Polynomials and the results are interpreted in terms of molecular interactions present in the mixtures. Keywords: adiabatic compressibility, free length, free volume, acoustic impedance, internal pressure, molar volume, excess values. 1. INTRODUCTION The study of molecular interaction in the liquid mixtures is of considerable in the elucidation of the structural properties of the molecules. The intermolecular interactions influence the structural arrangement along with the shape of the molecules. Dielectric relaxation studies of polar molecules in non-polar solvent using microwave absorption method have been widely used to study the molecular structures including the molecular interactions in liquid mixtures [1,2]. Since, acoustic parameters provide a better insight into molecular environments in liquid mixtures, it seemed important to study molecular interactions which motivated the authors to carry-out the present investigation in the ternary liquid mixtures of cresols (m- cresols, o-cresols and p-cresols) with N-N dimethyl formamide (DMF) in a non-polar solvent ccl 4 using ultrasonic technique. Apart from measuring the ultrasonic velocity, density and viscosity, other acoustical parameters and some of their excess values have also been evaluated for these ternary liquid mixtures at temperatures 303.308 and 313K, respectively. The following are the three ternary liquid systems which have been taken up for the present study, System-I o-cresols + CCl 4 + DMF System-II p-cresols + CCl 4 + DMF System-III m-cresols + CCl 4 + DMF 2. MATERIALS AND METHODS The chemicals CCl4, DMF, m- cresol, o- cresol, p- cresol used in the study were the products from S.D fine. Chem. Ltd and E-Merck. All compounds were of AR grade with minimum assay of 99.9%. Therefore all chemicals were used without further purification. The densities of pure liquids and their ternary mixtures were measured by using single capillary pycnometer (made of Borosil glass). The capillary, with graduated marks, had a uniform bore and could be closed by a well-fitting glass cap. The marks on the capillary were calibrated by using triple-distilled water. The densities of pure water at required temperatures were taken from the literature [3]. The accuracy in density measurements was found to be ±0.0001 kg m -3. The ultrasonic speeds in pure liquids and in their mixtures were measured by using a single-crystal variable-path ultrasonic interferometer [Mittal enterprises, New Delhi] operating at 3MHz with an accuracy of ±3ms -1. The viscosities of pure liquids and their binary mixtures were measured by using Ubbelohde-type suspended level viscometer. The viscometer was allowed to stand in a thermostatic water bath for 30 min so that the thermal fluctuations in viscometer were minimized. 3. THEORY AND CALCULATIONS The adiabatic compressibility is found by 1 β = (1) 2 ρu The free length (L f ) is given by the relation, L f = K T β 1/2 (2) Where K T is the temperature dependent constant. The free volume (V f ) is measured by using the relation, V M effu = Kη 3/ 2 f (3) Where M eff is the effective molecular weight (M eff = m i x i, in which m i and x i are the molecular weight and the mole fraction of the individual constituents respectively). The internal pressure is calculated by 1/ 2 2 / 3 Kη ρ π = brt 7 / 6 (4) i U M Where b stands for cubic packing which is assumed to be 2 for liquids and K is a dimensionless constant independent of temperature and nature of liquids and its value is 4.281x10 9, T is the absolute temperature and M eff is the effective molecular weight.where K is Boltzmann s constant and h is the Planck s constant. The specific acoustic impedance is given by 1

Z = Uρ (5) Excess parameters (A E ) by definition; represent the difference between the parameters of real mixtures Aexp and those corresponding to an ideal mixture Aid. A E = A exp - A id (6) Where A id = n i= 1 A X i i, Ai is any acoustical parameters and X i the mole fraction of the liquid components. The some of the excess properties of were fitted to Redlich-Kister [4] Polynomial, Where Y E refer to excess properties, x 1 and x 3 are the mole fraction of the components of the ternary mixtures. The coefficients (A i ) were obtained by fitting equation (8) to experimental values using a least square regression method. In each case, the optimal number of coefficients was ascertained from an approximation of the variation in the standard deviation (σ). The calculated values of A i (7) along with the tabulated standard deviations (σ) are listed in the Table-6. The standard deviation (σ) was calculated using the equation σ 2 = (8) Where n is the number of data points and m is the number of coefficients. 4. RESULTS AND DISCUSSIONS The values of density (ρ), Viscosity (η), ultrasonic velocity (u) were taken for the three systems at three temperatures are displayed in the Table-1. From these observed values various acoustical parameters like adiabatic compressibility (β), freelength (L f ), free volume (V f ), internal pressure (π i ), acoustic impedance(z), molar volume (V m ) have been evaluated and is presented in the Tables 2 and 3. The excess values of some of these acoustical parameters are also calculated and are displayed in the Tables 4 and 5. Table-1. Density (ρ), viscosity (η) and ultrasonic velocity (U) of. Mole fraction Density ρ/(kg/m 3 ) Viscosity η/( 10-3 NSm -2 ) Velocity U/(m/s) Temperature ( K) X 1 X 3 303 308 313 303 308 313 303 308 313 0.0000 0.6000 1229.40 1226.38 1221.23 0.8725 0.8473 0.7389 1149.47 1148.48 1021.20 0.1000 0.5000 1235.32 1233.24 1228.73 1.1054 1.0094 0.9393 1170.96 1156.8 1144.08 0.2000 0.4000 1237.31 1235.17 1230.41 1.3536 1.2778 1.1616 1176.20 1171.97 1151.16 0.3056 0.2871 1240.60 1237.12 1234.79 1.7348 1.6285 1.4868 1178.04 1172.67 1158.00 0.4000 0.2000 1243.30 1240.24 1236.21 1.9987 1.8902 1.5912 1179.33 1173.53 1159.63 0.4998 0.1001 1245.87 1241.08 1238.73 2.2548 2.0723 1.8097 1192.44 1178.78 1164.42 0.6000 0.0000 1248.01 1244.96 1240.54 2.5316 2.3148 2.001 1204.2 1197.06 1184.23 0.0000 0.6000 1229.40 1226.38 1222.23 0.8725 0.8203 0.7655 1159.3 1148.48 1121.20 0.1012 0.4942 1231.91 1229.20 1225.17 1.1413 1.0332 0.9831 1170.23 1161.48 1151.03 2

0.2000 0.4000 1239.75 1236.12 1230.21 1.3860 1.3585 1.2539 1183.13 1167.90 1153.98 0.3055 0.2871 1242.40 1239.34 1234.85 1.9790 1.8188 1.6306 1184.24 1168.93 1154.20 0.4000 0.19996 1244.16 1240.84 1237.26 2.3663 2.1431 1.9055 1187.20 1173.48 1161.30 0.4999 0.1001 1246.84 1243.12 1240.02 2.7801 2.4661 2.2108 1190.35 1177.82 1164.83 0.6000 0.0000 1248.63 1245.36 1242.24 3.0238 2.7263 2.3857 1195.4 1182.3 1166.54 I 0.0000 0.6000 1229.40 1226.38 1221.23 0.8725 0.8203 0.7655 1159.30 1148.48 1131.20 0.1001 0.4998 1232.32 1227.84 1224.50 1.0653 1.0068 0.8802 1169.67 1155.13 1147.98 0.1999 0.3999 1236.9 1232.16 1229.03 1.4222 1.3143 1.2243 1174.06 1165.03 1149.07 0.3000 0.2999 1241.02 1236.02 1231.62 1.7632 1.6587 1.5384 1179.18 1168.93 1150.5 0.3999 0.1999 1243.03 1238.03 1233.4 1.9521 1.8012 1.6946 1182.47 1174.32 1162.23 0.4998 0.1001 1246.8 1240.91 1237.06 2.339 2.2025 1.9653 1193.76 1182.08 1168.53 0.6000 0.0000 1247.67 1242.03 1239.5 2.7786 2.6496 2.3853 1209.26 1197.18 1185.75 In all the three liquid systems, the values of density (ρ), viscosity (η) and the ultrasonic velocity (U) increase with increasing molar concentration of cresols. Cresols are organic compounds which are methylphenols. They are a widely occurring natural and manufactured group of aromatic organic compounds which are categorized as phenols (sometimes called phenolics). Depending on the temperature, cresols can be solid or liquid because they have melting points not far from room temperature. Like other types of phenols, they are slowly oxidized by long exposure to air and the impurities often give cresols a yellowish to brownish red tint. Cresols have an odor characteristic to that of other simple phenols. In its chemical structure, a cresol molecule has a methyl group substituted onto the benzene ring of a phenol molecule. There are three forms of cresols that are only slightly different in their chemical structure: ortho-cresol (ocresol), meta-cresol (m-cresol), and para-cresol (p-cresol). O-Cresol p-cresol m-cresol Cresols are isomeric substituted phenols with a methyl substituent at one of the o-, m-, or p- positions relative to the OH-group. Physically, they are white crystalline solids or yellowish liquids with a strong phenol-like odour. The compounds are highly flammable, moderately soluble in water and soluble in ethanol, ether, acetone, or alkali hydroxides. Chemically, these alkylphenols undergo electro-philic substitution reactions at the vacant o- or p- positions or undergo condensation reactions with aldehydes, ketones, or dienes. This chemical interaction may involve the association due to hydrogen bonding or due to dipoledipole interaction or may be due to the formation chargetransfer complexes. All these processes may lead to strong interaction forces. [5]. since ortho, Meta, and para cresols structurally similar, the increase in velocity in these liquid mixtures suggest that strong molecular interaction between 3

the cresols and DMF. The forces responsible for these interactions may probably be dipole-induced dipole or may be due to hydrogen bonding. [6]. The increase in velocity further may also be interpreted as the concentration of cresols is increased, since DMF is polar (hydrophilic) aprotic solvent with high boiling point, it can miscible with water and majority of organic liquids, belonging to amide group, the attached methyl group of (- CH 3 ) in o-cresol has its own effect as well as hyperconjugate effect. Hence, due to the presence of methyl group, the removal of proton in o-cresol is not facilitated as quickly as in ccl 4. Thus cresol molecules may form hydrogen bonds with DMF molecules more readily, giving rise to increase in velocity. Further, due to the addition of -CH 3 group at ortho position in the ring, molecular association taking place between DMF and cresol molecules through hydrogen bonding [6]. The dilute solutions minimize the effect of viscosity, internal field etc., therefore, for dilution apolar solvents like carbontetrachloride (CCl 4 ), benzene (C 6 H 6 ) and cyclohexane etc., are used. Normally apolar solvents provide the medium and dilution for the mixture, which in turn, also minimizes the requirement of pure liquids in large quantity. Hence, in the present investigation, ccl 4 is used. Also, as CCl 4 is a non-polar solvent which is not taking part in the reaction, so the mole fraction of ccl 4 does not influence the mixture. [7] Adiabatic compressibility β is found to be decreased with increasing concentration of cresols. It is primarily the compressibility that changes with structure which leads to change in ultrasonic velocity. The change in adiabatic compressibility (β) in liquid mixtures indicates there is a definite contraction on mixing and the variation is may be due to complex formation. This clearly shows that there is significant interaction between the DMF-cresol molecules. [8] Intermolecular free length (L f ) shows a similar behavior as reflected by adiabatic compressibility. The decrease in compressibility brings the molecules to a closer packing resulting into a decrease of intermolecular free length. Intermolecular free length (L f ) is a predominant factor in determining the variations of ultrasonic velocity (U) in the mixtures. As L f increases, U decreases and vice-versa, showing an inverse behavior. The interdependence of L f and U has been evolved from model by Eyring and Kincaid [9]. The decrease in the values of adiabatic compressibility and the free length with increase in ultrasonic velocity (U) further strengthens the strong molecular association between the unlike molecules through hydrogen bonding. Table-2. Adiabatic compressibility (β), free length (L f ) free volume (V f ) and internal pressure (π i ) of. Mole fraction β/( 10 10 m 2 N -1 ) L f /( 10-10 m) V f /( 10 7 m 3 mol 1 ) π i /( 10 6 Nm 2 ) Temperature ( K) X 1 X 3 303 308 313 303 308 313 303 308 313 303 308 313 0.0000 0.6000 6.0522 6.1820 6.5085 0.4909 0.5006 0.5179 1.8713 2.0241 2.1658 464.3028 459.0221 455.0376 0.1012 0.4942 5.9276 6.0305 6.1607 0.4858 0.4939 0.5039 1.3401 1.5384 1.6351 507.1634 491.6287 488.4774 0.2000 0.4000 5.7624 5.9310 6.1041 0.4789 0.4898 0.5016 1.0593 1.0706 1.1858 541.1838 547.0931 535.6310 0.3055 0.2871 5.7393 5.9052 6.0789 0.4780 0.4887 0.5005 0.6589 0.7333 0.8476 618.7299 605.8803 585.2741 0.4000 0.19996 5.7026 5.8524 5.9931 0.4765 0.4865 0.4970 0.5236 0.5970 0.7010 658.3889 639.4749 614.7878 0.4999 0.1001 5.6603 5.7987 5.9436 0.4747 0.4843 0.4949 0.4311 0.5079 0.5885 690.0555 662.8201 640.2364 0.6000 0.0000 5.6045 5.7445 5.9156 0.4724 0.4821 0.4938 0.3990 0.4584 0.5488 695.6014 673.9203 643.8837 4

0.0000 0.6000 6.0522 6.1820 6.5138 0.4909 0.5006 0.5182 1.8713 2.0241 2.1658 464.3028 459.0221 454.7881 0.1000 0.5000 5.9039 6.0595 6.2177 0.4848 0.4951 0.5062 1.3991 1.5744 1.7251 502.1282 490.1693 481.9979 0.2000 0.4000 5.8420 5.8944 6.1331 0.4823 0.4883 0.5028 1.0900 1.1821 1.3276 534.8676 528.5904 515.4382 0.3056 0.2871 5.8083 5.8781 6.0393 0.4809 0.4876 0.4989 0.7965 0.8698 0.9784 580.2178 571.6669 557.8971 0.4000 0.2000 5.7830 5.8547 6.0155 0.4798 0.4866 0.4979 0.6678 0.7208 0.9167 606.8182 600.3441 561.8789 0.4998 0.1001 5.6449 5.7988 5.9539 0.4741 0.4843 0.4954 0.5916 0.6600 0.7940 620.7110 606.8074 579.0706 0.6000 0.0000 5.5257 5.6055 5.7480 0.4690 0.4762 0.4867 0.5265 0.5968 0.7307 634.0063 617.0782 584.7978 I 0.0000 0.6000 6.0522 6.1820 6.3992 0.4909 0.5001 0.5136 1.8713 2.0241 2.1948 464.3028 459.0221 452.7734 0.1001 0.4998 5.9313 6.1037 6.1969 0.4859 0.4968 0.5054 1.4766 1.5773 1.9116 492.3581 488.4063 464.6753 0.1999 0.3999 5.8652 5.9794 6.1623 0.4832 0.4917 0.5040 1.0092 1.1229 1.2234 548.7212 536.8910 529.3363 0.3000 0.2999 5.7951 5.9210 6.1341 0.4803 0.4893 0.5028 0.7706 0.8336 0.9112 589.4618 582.1273 572.8958 0.3999 0.1999 5.7536 5.8573 6.0022 0.4786 0.4867 0.4974 0.6947 0.7757 0.8369 598.8021 585.1273 578.3005 0.4998 0.1001 5.6282 5.7672 5.9201 0.4734 0.4830 0.4940 0.5610 0.6049 0.7054 632.0867 624.5753 601.7751 0.6000 0.0000 5.4810 5.6176 5.7381 0.4671 0.4767 0.4863 0.4608 0.4875 0.5625 662.6470 659.0665 637.6672 It is observed that for all the three liquid systems, the values free volume of (V f ) decrease and the internal pressure (π i ) increase. Further, the decrease in free volume and increase in internal pressure with rise in concentration of cresols in all the systems clearly show the increasing magnitude of interactions [10]. Such an increase in internal pressure generally indicates association through hydrogen bonding [11] and hence supports the present investigation. Further, in all three liquid systems, the values of acoustic impedance (Z) are found to be increased. When an acoustic wave travels in a medium, there is a variation of pressure from particle to particle. The ratio of the instantaneous pressure excess at any particle of the medium to the instantaneous velocity of that particle is known as specific acoustic impedance of the medium. This factor is governed by the inertial and elastic properties of the medium. It is important to examine specific acoustic impedance in relation to concentration and temperature. When a plane ultrasonic wave is set up in a liquid, the pressure and hence density and refractive index show specific variations with distance from the source along the direction of propagation. In the present investigation, it is observed that these acoustic impedance (Z) values increase with increasing concentration of cresols. Such an increasing values of acoustic impedance (Z) further supports the possibility of molecular interactions due to H-bonding between the DMF-cresol molecules. It is seen from the Table-3, the values of molar 5

volume (V m ) increases with increase in concentration of cresols in all the three liquid systems. This is because of the fact molecular weight is directly proportional to the molar volume. The molecular weights of cresols, DMF respectively are 108.14, 73.09. Since cresols are having higher molecular weights in the solution comparing DMF (as CCl 4 is a non-polar solvent, which do not taking part in the reaction) whose concentration are increasing in the mixture which supports the calculation. Moreover, molar volume (V m ) is also increases with rise in temperature in the present study, which may probably would be caused from the fact that thermal energy facilitates an increase in the molecular separation in the liquid mixtures which leads to an increase in molar volume (V m ) with elevation of temperature. Table-3. Acoustic impedance (z) and molar volume (V m ) of. Mole fraction Acoustic impedance Z x 10 6 kg m 2 /s Temperature ( K) Molar volume (V m ) x 10-5 m 3 X 1 X 3 303 308 303 303 308 313 0.0000 0.6000 1.4252 1.4085 8.5721 0.1925 0.1958 0.1990 0.1012 0.4942 1.4416 1.4277 8.8731 0.1915 0.1949 0.1981 0.2000 0.4000 1.4668 1.4437 9.0541 0.1908 0.1938 0.1971 0.3055 0.2871 1.4713 1.4487 9.3911 0.1893 0.1926 0.1960 0.4000 0.19996 1.4771 1.4561 9.5968 0.1886 0.1919 0.1954 0.4999 0.1001 1.4842 1.4642 9.8569 0.1879 0.1914 0.1948 0.6000 0.0000 1.4926 1.4724 10.1238 0.1876 0.1910 0.1944 0.0000 0.6000 1.4252 1.4085 8.5721 0.1925 0.1958 0.1990 0.1000 0.5000 1.4465 1.4266 8.8148 0.1916 0.1950 0.1983 0.2000 0.4000 1.4553 1.4476 9.0839 0.1908 0.1941 0.1974 0.3056 0.2871 1.4615 1.4507 9.4053 0.1898 0.1931 0.1964 0.4000 0.2000 1.4663 1.4555 9.6035 0.1892 0.1925 0.1961 0.4998 0.1001 1.4856 1.4630 9.8629 0.1888 0.1921 0.1956 0.6000 0.0000 1.5029 1.4903 10.1279 0.1884 0.1918 0.1954 I 0.0000 0.6000 1.4252 1.4085 8.5721 0.1925 0.1958 0.1990 0.1001 0.4998 1.4414 1.4183 8.8370 0.1918 0.1950 0.1986 0.1999 0.3999 1.4522 1.4355 9.0856 0.1906 0.1939 0.1972 0.3000 0.2999 1.4634 1.4448 9.3383 0.1897 0.1930 0.1962 6

0.3999 0.1999 1.4698 1.4538 9.6059 0.1893 0.1927 0.1959 0.4998 0.1001 1.4884 1.4669 9.8565 0.1886 0.1919 0.1953 0.6000 0.0000 1.5088 1.4869 10.1314 0.1881 0.1912 0.1946 In order to understand the nature of molecular interactions between the components of the liquid mixtures, it is of interest to discuss the same in term of excess parameter rather than actual values. Non-ideal liquid mixtures show considerable deviation from linearity in their physical behavior with respect to concentration and these have been interpreted as arising from the presence of strong or weak interactions. The extent of deviation depends upon the nature of the constituents and composition of the mixtures. It is learnt that the dispersion forces are responsible for possessing positive excess values, while dipole-dipole, dipole- induced dipole, charge transfer interaction and hydrogen bonding between unlike molecules are responsible for possessing negative excess values [5] Table-4. Excess values of adiabatic compressibility (β), free length (L f ), free volume (V f ) and internal pressure (π i ) of. Mole fraction Excess adiabatic compressibility (β E 10 10 m 2 N -1 )) Excess free length (L E f 10 --12 m) Excess free volume (V E f 10 7 m 3 mol 1 ) Excess internal pressure (π E i 10 6 Nm 2 ) Temperature ( K) X 1 X 3 303 308 313 303 308 313 303 308 313 303 308 313 0.0000 0.6000-0.212-0.237-0.227-0.581-0.650-0.622-0.180-0.170-0.187-10.885-9.706-10.315 0.1001 0.4998-0.425-0.480-0.645-1.460-1.649-2.315-0.660-0.610-0.669-52.892-42.573-43.866 0.1999 0.3999-0.611-0.614-0.724-2.213-2.189-2.624-0.827-0.933-0.973-78.749-86.677-81.171 0.3000 0.2999-0.714-0.731-0.823-2.667-2.696-3.051-1.024-1.074-1.113-128.070-121.868-110.736 0.3999 0.1999-0.770-0.802-0.899-2.908-3.005-3.376-0.987-1.032-1.075-139.331-130.288-118.218 0.4998 0.1001-0.843-0.888-0.963-3.219-3.369-3.645-0.898-0.935-0.987-138.758-126.995-117.980 0.6000 0.0000-0.913-0.964-1.009-3.518-3.689-3.837-0.766-0.805-0.847-121.372-114.108-103.909 0.0000 0.6000-0.212-0.237-0.222-0.581-0.650-0.601-0.180-0.170-0.187-10.885-9.706-10.066 0.1001 0.4998-0.433-0.440-0.580-1.493-1.485-2.051-0.605-0.576-0.586-47.919-40.809-37.586 0.1999 0.3999-0.554-0.651-0.709-2.003-2.365-2.586-0.804-0.846-0.862-73.320-71.502-64.648 0.3000 0.2999-0.667-0.750-0.851-2.471-2.777-3.168-0.929-0.979-1.022-101.284-98.069-91.685 7

0.3999 0.1999-0.721-0.801-0.886-2.708-3.000-3.322-0.901-0.958-0.945-108.373-106.794-86.457 0.4998 0.1001-0.849-0.887-0.957-3.243-3.359-3.614-0.818-0.859-0.884-104.168-99.071-87.476 0.6000 0.0000-0.944-1.018-1.075-3.647-3.919-4.114-0.715-0.749-0.774-96.766-91.402-80.306 I 0.0000 0.6000-0.212-0.237-0.336-0.581-0.650-1.059-0.180-0.170-0.158-10.885-9.706-8.051 0.1001 0.4998-0.408-0.400-0.599-1.393-1.324-2.128-0.535-0.573-0.418-39.132-39.228-22.004 0.1999 0.3999-0.535-0.582-0.685-1.919-2.077-2.482-0.869-0.893-0.945-84.479-78.217-75.841 0.3000 0.2999-0.652-0.695-0.761-2.413-2.551-2.800-0.949-1.007-1.072-107.528-105.148-101.891 0.3999 0.1999-0.739-0.800-0.894-2.782-2.995-3.355-0.884-0.925-0.993-103.562-97.663-96.309 0.4998 0.1001-0.858-0.903-0.975-3.282-3.430-3.690-0.833-0.887-0.928-109.827-107.927-98.802 0.6000 0.0000-0.962-1.014-1.080-3.727-3.902-4.135-0.742-0.793-0.842-108.199-108.174-101.430 In the present investigation, the excess adiabatic compressibility (β E ) the excess free length (L f E ) and excess free volume (V f E ) exhibit negative values over the entire range composition in all the three liquid systems clearly indicating the presence of strong hydrogen bonding interactions between unlike molecules. This is in conformity with earlier workers [5, 12]. The strength of the interaction between the component molecules increase, when excess values tend to become increasingly negative. This also may be quantitatively interpreted in terms of closer approach of unlike molecules leading to reductions in compressibility and volume [6]. Further, the excess internal pressure (π i E ) which is usually described in terms of molecular interaction, whose negative excess values for all the liquid systems suggest that strong molecular association between the unlike molecules. The excess values of acoustic impedance (Z E ) which are furnished in Table5 are all positive in the liquid systems over the entire range of composition. The positive excess values of Z E clearly suggest that there is a strong molecular interaction existing between the DMF-cresol molecules [13]. The excess viscosity (η E ) values whose positive excess values for all the three liquid systems clearly supports this prediction [13]. Similar observations were observed by earlier workers [7, 14] supports the present investigation. Table-5. Excess Values of molar volume(v m E ), viscosity( η E ) and acoustic Impedance(Z E ) of. Mole fraction Excess molar volume V m E x10-5 m 3 mol 1 Excess viscosity η E x 10-5 NSm -2 Temperature ( K) Excess acoustic impedance Z E 104 kg m 2 /s X 1 X 3 303 308 313 303 308 313 303 308 313 0.0000 0.6000 2.0117 2.0040 1.9976 0.8717 0.8195 0.7648 5.7062-12.0060 40.5761 8

0.1012 0.4942 2.2166 2.2084 2.2042 1.1405 1.0324 0.9824 6.3710 2.5280 56.5902 0.2000 0.4000 2.2446 2.2431 2.2521 1.3851 1.3576 1.2531 7.6016 16.8358 70.0438 0.3055 0.2871 2.3634 2.3600 2.3632 1.9778 1.8177 1.6296 6.4783 30.8643 85.8758 0.4000 0.19996 2.3123 2.3111 2.3115 2.3649 2.1418 1.9043 5.6728 43.9770 98.8535 0.4999 0.1001 2.2613 2.2624 2.2633 2.7783 2.4645 2.2093 4.7065 57.7175 113.4112 0.6000 0.0000 2.1607 2.1607 2.1643 3.0216 2.7243 2.3840 3.6673 71.4960 127.8685 0.0000 0.6000 2.0117 2.0040 2.0047 0.8717 0.8196 0.7648 5.7062-12.0060 40.5313 0.1000 0.5000 2.1516 2.1391 2.1376 1.1046 1.0086 0.9386 6.8523 2.3829 55.6078 0.2000 0.4000 2.2638 2.2536 2.2559 1.3527 1.2769 1.1608 6.5505 16.9132 69.8296 0.3056 0.2871 2.3726 2.3715 2.3632 1.7337 1.6275 1.4858 5.7860 30.9810 86.2016 0.4000 0.2000 2.3161 2.3137 2.3162 1.9974 1.8890 1.5901 5.0205 43.9343 98.5849 0.4998 0.1001 2.2656 2.2710 2.2689 2.2533 2.0709 1.8084 4.7708 57.6414 113.2159 0.6000 0.0000 2.1627 2.1620 2.1699 2.5297 2.3131 1.9995 4.0731 72.5823 129.8649 I 0.0000 0.6000 2.0117 2.0040 2.0047 0.8717 0.8195 0.7648 5.7305-11.9796 41.0462 0.1001 0.4998 2.1715 2.1747 2.1658 1.0645 1.0060 0.8795 6.3780 1.8882 55.6151 0.1999 0.3999 2.2664 2.2716 2.2643 1.4213 1.3134 1.2235 6.2635 16.1471 69.5354 0.3000 0.2999 2.3130 2.3197 2.3221 1.7621 1.6577 1.5374 6.0358 30.0378 83.5772 0.3999 0.1999 2.3175 2.3241 2.3296 1.9508 1.8000 1.6935 5.2342 43.8340 98.5818 0.4998 0.1001 2.2620 2.2718 2.2758 2.3374 2.2010 1.9639 5.4159 62.3099 113.0053 9

0.6000 0.0000 2.1638 2.1716 2.1733 2.7766 2.6477 2.3836 4.2556 72.3663 129.9246 Table-6. Redlich Kister coefficients and standard deviation (σ) values. β E E L f E V f E V m I I I I Temperature a o a 1 a 2 σ 303-17.8694-47.7994-1430.08 0.4933 308-18.7402-30.7605-1376.95 0.5209 313-23.4139-108.87-1884.71 0.5692 303-18.6817-70.5868-1522.62 0.4846 308-20.8359-57.1756-1418.02 0.5230 313-24.2421-87.3599-1633.56 0.5512 303-19.7389-48.7874-1315.14 0.4688 308-20.6026-64.0679-1488.65 0.4973 313-25.14-123.467-1872.78 0.5219 303-63.4397-103.05-5134.6 1.8876 308-65.7152-22.052-4814.44 1.9781 313-84.4055-343.709-6855.96 2.1458 303-66.8333-198.465-5519.3 1.8494 308-74.3828-131.395-4979.48 1.9870 313-87.8587-257.168-5828.95 2.0857 303-70.8033-99.4602-4626.78 1.7838 308-72.9785-151.215-5240.59 1.8759 313-91.0755-395.999-6777.49 1.9599 303-27.0095-75.3797-1136.07 0.3820 308-28.2843-79.1603-1217.94 0.4062 313-27.3844 11.8088-712.78 0.4363 303-26.633-70.9515-1110.23 0.3706 308-27.1903-41.2753-970.838 0.3844 313-27.9636-55.1169-1067.15 0.3994 303-28.2539-52.4497-1088.34 0.3978 308-29.6638-46.5683-1057.59 0.4115 313-31.3325-68.5187-1250.78 0.4343 303 79.7109 596.743 5599.46 1.50345 308 79.8639 595.396 5599.85 1.50365 313 79.8408 595.224 5599.87 1.50425 303 80.3495 557.761 5273.41 1.50067 308 80.0065 552.278 5262.83 1.49741 313 79.957 552.284 5262.83 1.50036 303 80.71 572.443 5351.44 1.50522 308 80.6262 572.384 5351.44 1.50209 313 80.7014 572.354 5351.45 1.50041 10

η E I 303 47.5024 134.458 3953.38 1.4570 308 44.449 139.528 3811.32 1.3883 313 40.469 72.7464 3023.54 1.2529 303 46.2351 83.7455 3525.97 1.3416 308 43.0797 50.723 3044.09 1.2298 313 39.7901 98.7579 2897.24 1.0738 303 47.9384-16.8147 3927.51 1.5766 308 45.4072 6.45402 3498.43 1.4243 313 42.1973 53.1523 3390.84 1.2541 5. CONCLUSIONS From the data s of ultrasonic velocity, density and viscosity, related acoustical parameters and some of their excess values for the ternary liquid mixtures of o- cresols, p-cresols, m-cresols with DMF in carbon tetrachloride (CCl 4 ) at 303, 308 and 313 K, it is very obvious that there exist a strong molecular interaction existing between the unlike molecules. The cresols such as o-cresols, p-cresols and m-cresols form strong hydrogen bonding with DMF. However, no complex formation or charge-transfer reactions were observed in the present study. The molecular interaction is stronger in DMFcresols than in cresols- CCl 4 and in DMF-CCl 4 ACKNOWLEDGEMENTS The authors are thankful to Dr. A.N. Kannappan, Professor and Head, Department of Physics, Annamalai University for encouraging them. REFERENCES [1] P. J. Singh and K. S. Sharma. 1996. Dielectric behaviour of ketone-amine binary mixtures at microwave frequencies Pramana. 46: 259-270. [8] K. Mohankrishnan, K. Rambabu, D. 1995. Ramachandran and G.K. Raman. Phys. Chem. Liq. (UK). 29: 257. [9] H. Erying and J. F. Kincaid. 1928. Free Volumes and Free Angle Ratios of Molecules in Liquids. J. Chem. Phys (USA). 6: 620-629. [10] D. Anbhananthan. J. 1979. Acoust. Soc. India. 7: 123. [11] V. Rajendran, V. 1994. Ind. J. Pure and Appl. Phy. 32: 523. [12] S. N. Gour, J. S Tomar and R. P. Varma. 1986. Ind. J. Pure Appl. Phys. 24: 602. [13] Jong-Rim Bae and Seung Yun. 1998. Ultrasonic Velocity and Absorption in Binary Solutions of Silicon Dioxide and Water. Jpn. J. App Phys. 37: 2801-2802. [14] R. Singh, J.P. Mishra and M. C. Shukla, Saxena. 1983. J. Mol. Liq. (Netherlands). 26: 29. [2] M. Jorg, A. Ghoneim S. G. 1995. Turley and M. Stockhausen. Phys. Chem. Liq. (UK). 29: 263. [3] S. L. Abd-EL-Messieh. 1996. Indian J. Phys. 70B (2): 119. [4] O. Redlich and A. T. Kister. 1940. Ind. Eng. Chem. 40: 345. [5] R. J Fort and M. W. R. Moore. 1965. Trans. Faraday Soc. [6] A. Jayakumar, S. Karunanithi and V. Kannappan. 1996. Ind. J. Pure Appl. Phys. 34: 761. [7] P. Aasthees Awasthi and J. P Shukla. 2003. Ultrasonic and IR study of intermolecular association through hydrogen bonding in ternary liquid mixtures Ultrasonics. 10: 241-246 11